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Calculating percent yield

Chemistry
Tutor: None Selected Time limit: 1 Day

Methane (CH4, 16.05 g/mol) reacts with oxygen to form carbon dioxide (CO2, 44.01 g/mol) and water (H2O, 18.02 g/mol). Assume that you design a system for converting methane to carbon dioxide and water. To test the efficiency of the system in the laboratory, you burn 5.00 g methane. The actual yield is 6.10 g water. What is your percent yield?

Apr 13th, 2015

The first step is to write a balanced chemical reaction for this situation.

CH4 + 2 O2 ====> CO2 + 2 H2O

The next step will be to calculate the theoretical yield of water from the reaction of 5 g methane.

5.00 g CH4 * 1 mol CH4 / 16.05 g * 2 mol H2O / 1 mol CH4 * 18.02 g H2O / 1 mol = 11.227 g

Now we can calculated the percent yield

% yield = actual yield / theoretical yield * 100%

% yield = 6.10 g / 11.227 g * 100%

% yield = 54.3 %

Apr 13th, 2015

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Apr 13th, 2015
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